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Syllabus

_{c}) for the reaction $2HCl\left(g\right)\leftrightarrow {H}_{2}\left(G\right)+C{l}_{2}\left(g\right)$ is 4*10^{-34}at 25^{o}C.What is the equilibrium constant for the reaction $\frac{1}{2}{H}_{2}\left(g\right)+\frac{1}{2}C{l}_{2}\left(g\right)\leftrightarrow HCl\left(g\right)$

(1) 2*10

^{-17}(2) 2.5*10^{33 }(3) 5*10^{6}(4) NOTIn above reaction at equilibrium condition mole fraction of PCl

_{5}is 0.4 and mole fraction of Cl_{2}is 0.3. Then find out mole fraction of PCl_{3}.1. 0.3 2. 0.7 3. 0.4 4. 0.6

25.When heating PCl_{5}then it decompose PCl_{3}and Cl_{2}in form of gas, The vapour density of gas mixture is 70.2 and 57.9 at 200$\xb0$ C and 250$\xb0$ C. The degree of dissociation of PCl_{5}at 200$\xb0$ C and 250$\xb0$ C is(1) 48.50% & 80% (2) 60% & 70%

(3) 70% & 80% (4) 80% & 90%

_{p}will be(1) 3 P (2) 2 P (3) $\frac{\mathrm{P}}{3}$ (4) $\frac{\mathrm{P}}{2}$

_{p}for the reaction ${\mathrm{N}}_{2}{\mathrm{O}}_{4}\rightleftharpoons 2{\mathrm{NO}}_{2}$is 0.66 then what is the equilibrium pressure of N_{2}O_{4}. (Total pressure at equilibrium is 0.5 atm)(1) 0.168 (2) 0.322 (3) 0.1 (4) 0.5

answer- 7.559 ? 10-6

43. Evaluate K

_{p}for the reaction : H_{2}+ I_{2}$\rightleftharpoons $ 2HI, If 2 moles each of H_{2}and I_{2}are taken initially. The equilibrium moles of HI are 2.(1) 2.5 (2) 4 (3) 0.25 (4) 1.0

Q). At $90\xb0C$, the pH of 0.1 M NaCl aqueous solution is :-

(1) < 7

(2) > 7

(3) 7

(4) 0.1

_{2}can be expressed as 2CO_{2}$\rightleftharpoons 2CO+{O}_{2}$. If the 2 mol of CO_{2}is taken initially and 40% of the CO_{2}is disscoiatated completely. What is the total number of moles at equilibrium:-$1.2.42.2.03.1.24.$5

if the equilibrium concentration are [N2O4]=0.75 and [NO2]=0.062M, R=0.08206L at K-1 mol-1

Ans:AC.

Explain how?

Q121. Following five solution of KOH were prepare as-

First $\to $ 0.1 moles in 1 L

Second $\to $ 0.2 moles in 2 L

Third $\to $ 0.3 moles in 3 L

Fourth $\to $ 0.4 moles in 4 L

Fifth $\to $ 0.5 moles in 5 L

The pH of resultant solution is :-

(1) 2 (2) 1 (3) 13 (4) 7

Q. How many moles per litre of $PC{l}_{5}$ has to be taken to obtain 0.1 mol of $C{l}_{2}$, if the value of equilibrium constant ${K}_{c}$ is 0.04?

(1) 0.15

(2) 0.25

(3) 0.35

(4) 0.05

in a 500 ml capacity vessel CO and Cl2 are mixed to form COCL2.at euilibrium,it contains 0.2 moles of COCl2 and 0.1 mole of each of CO and CO2 the euilibrium constant Kc for the reaction CO+Cl2----- COCL2 is

_{2}are mixed with two moles of gas B_{2}in a flask of volume 1 lit. If at equilibrium 0.5 moles of A_{2}are obtained. Then find out K_{p}for reactionA

_{2}(g) + B_{2}(g) ⇌ 2AB(g)(1) 12 (2) 9 (3) 4 (4) 36

Q. 0.05 M ammonium hydroxide solution is dissolved in 0.001 M ammonium chloride solution . What will be the $O{H}^{-}$ ion concentration of this solution : ${K}_{b}\left(N{H}_{4}OH\right)=1.8\times {10}^{-5}$

$\left(1\right)3.0\times {10}^{-3}\left(2\right)9.0\times {10}^{-4}\phantom{\rule{0ex}{0ex}}\left(3\right)9.0\times {10}^{-3}\left(4\right)3.0\times {10}^{-4}$

Can you show the corresponding reactions pls

31. A 1 M solution of glucose reaches dissociation equilibrium according to equation given below $6HCHO\rightleftharpoons {C}_{6}{H}_{12}{O}_{6}$. What is the concentration of HCHO at equilibrium if equilibrium constant is 6 x 10

^{22}(a) 1.6 x 10

^{-8}M (b) 3.2 x 10^{-6}M(c) 3.2 x 10

^{-4}M (d) 1.6 x 10^{-4 M}$\mathbf{23}\mathbf{.}{X}_{2}+{Y}_{2}\rightleftharpoons 2XYreactionwasstudiedatcertaintemperature.Inthebeginning1moleof{X}_{2}wastakeninaonelitreflaskand2molesof{Y}_{2}wastakeninanother2litreflask.Whatistheequilibriumconcentrationof{X}_{2}and{Y}_{2}?(Givenequilibriumconcentrationof\left[XY\right]0.6mol{L}^{-1}).\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\left(1\right)\left(\frac{1}{3}-0.3\right),\left(\frac{2}{3}-0.3\right)\left(2\right)\left(\frac{1}{3}-0.6\right),\left(\frac{2}{3}-0.6\right)\phantom{\rule{0ex}{0ex}}\left(3\right)\left(1-0.3\right),\left(2-0.3\right)\left(4\right)\left(1-0.6\right),\left(2-0.6\right)$

answer- 10 raised 10

Q.168. Calculate the pH of a buffer solution prepared by dissolving 30 g of $N{a}_{2}C{O}_{3}$ in 500 mL of an aqueous solution containing 150 mL of 1 M HCl. Ka for

$HC{{O}_{3}}^{-}=5.63\times {10}^{-11}\left[\mathrm{log}\left(\frac{133}{150}\right)=-0.05\right]$

(1) 8.197

(2) 9.197

(3) 10.197

(4) 11.197

Illustration 1

CH3COOH + H

_{2}O $\rightleftharpoons $CH_{3}COO^{-}+ H30^{+}; K_{1}= 1.8 x 10^{-5}2H

_{2}O $\rightleftharpoons $ H_{3O}^{+ }+ OH^{-}; K_{2}= 1 x 10^{-14}Calculate equilibrium constant for

CH

_{3}COOH + OH^{-}$\rightleftharpoons $ CH_{3}COO^{-}+ H_{2}O1. More in 5 litre vessel 2. More in 10 litre vessel 3. Equal in both vessel 4. None of these

For a reaction, $2S{O}_{2\left(g\right)}+{O}_{2\left(g\right)}\iff 2S{O}_{3\left(g\right)}$ , 1.5 moles of $S{O}_{2}$ and 1 mole of ${O}_{2}$ are taken in a 2 L vessel. At equilibrium the concentration of $S{O}_{3}$ was found to be 0.35 mol ${L}^{-1}$. The for the reaction would be

Q. Fixed volume of 0.1 M benzoic acid (pK

_{a}= 4.2) solution is added into 0.2 M sodium benzoate solution and formed a 300 mL. resulting acidic buffer solution. If pH of the resulting solution is 3.9, then added volume of benzoic acid is(a) 240 mL (b) 150 mL

(c) 100 mL (d) None

^{-1}^{-1}^{-1}time^{-1}The half life of A in the reaction is:

(A) 1.386 min

(B) 1.386 min

(C) 0.01 min

(D) 0.01 min

1. One mole of N

_{2}O_{4}(g) in a 1 L flask decornposes to attain the equilibrium N_{2}O_{4}(g) $\rightleftharpoons $2NO_{2}(g)At the equilibrium the mole fraction of NO

_{2}is 1/2 Hence K_{c}will be:(1) 1/3 (2) 1/2 (3) 2/3 (4) 1

^{-16}% of the reactant molecules exist in the activated state, the E_{a}( activation energy ) of the reaction is(a) 12 kJ/mole (b) 831.4 kJ/mole (c) 100 kJ/mole (d) 88.57 kJ/mole

Q7. In a reaction 2HI $\to $H

_{2}+ I_{2, }the concentration of HI decrease from 0.5 ml L^{–1}to 0.4 mol L^{–1}in 10 minutes. What is the rate of reaction during this interval?(a) 5 × 10

^{–3}M min^{–1}(b) 2.5 × 10^{–3}M min^{–1}(c) 5 × 10

^{–2}M min^{–1}(d) 2.5 × 10^{–2}M min^{–1}_{c}= 9. If A and B are taken in equal amounts, then amount of C at equilibrium is :(1) 1 (2) 0.25 (3) 0.75 (4) None of these

Ans: C.

Expln pls asap

21. At 550 K, the K

_{c}for the following reaction is 10^{4}mol^{-1}L.X

_{(g) }+Y_{(g)}$\rightleftharpoons $Z_{(g)}At equilibrium, it was observed that

$\left[\mathrm{X}\right]=\frac{1}{2}\left[\mathrm{Y}\right]=\frac{1}{2}\left[\mathrm{Z}\right]$

What is the value of [Z] ( in mol L

^{-1}) at equilibrium ?(a) 2 x 10

^{-4}(b) 10^{-4}(c) 2 x 10^{-4 }(d) 10^{4}Q. Two sample of HI each of 5 gm. were taken seperately into vessels of volume 5 and 10 litres respectively at 27$\xb0$C. The extent of dissociation of HI will be :-

(1) More in 5 litre vessel

(2) More in 10 litre vessel

(3) Equal in both vessel

(4) None of these

_{3}COONa + 1 mole of HCl per litre and of other solution containing 1 mole CH_{3}COONa + 1 mole of acetic acid per litre(1) 1 : 1 (2) 2 : 1 (3) 1 : 2 (4) 2 : 3

Q.3. For the reaction,

$2CO\left(g\right)+{O}_{2}\left(g\right)\to 2C{O}_{2}\left(g\right);\u2206H=-560kJmo{l}^{-1}$

In one litre vessel at 500 K the initial pressure is 70 atm and after the reaction it becomes 40 atm at constant volume of one litre. Calculate change in internal energy. All the above gases show significant deviation from ideal behaviour. (1 Latm = 0.1 kJ)

$\mathbf{25}\mathbf{.}Considerthegeneralhypotheticalreaction,\phantom{\rule{0ex}{0ex}}{A}_{\left(s\right)}\rightleftharpoons 2{B}_{\left(g\right)}+3{C}_{\left(g\right)}\phantom{\rule{0ex}{0ex}}IftheconcentrationofCatequilibriumisdoubled,thenaftertheequilibriumisre-established,theconcentrationofBwillbe\phantom{\rule{0ex}{0ex}}\left(a\right)twotimestheoriginalvalue\phantom{\rule{0ex}{0ex}}\left(b\right)onehalfofitsoriginalvalue\phantom{\rule{0ex}{0ex}}\left(c\right)1/2\sqrt{2}timestheoriginalvalue\phantom{\rule{0ex}{0ex}}\left(d\right)2\sqrt{2}timestheoriginalvalue.$

What does

Threshold Energymean?11. For I

_{2}(g) $\rightleftharpoons $2I(g), K_{C}at 1000 K is 10^{-6}. One mole I_{2}is added in a one-litre container. Which of the following expressions is correct for the above system at equilibrium ?$\left(1\right)\left[{\mathrm{I}}_{2}\right]+\left[\mathrm{I}\right]=1+\mathrm{x}\left(2\right)\left[{\mathrm{I}}_{2}\right]=\frac{1}{2}\left[\mathrm{I}\right]\phantom{\rule{0ex}{0ex}}\left(3\right)\left[{\mathrm{I}}_{2}\left(\mathrm{g}\right)\right]\left[\mathrm{I}\left(\mathrm{g}\right)\right]\left(4\right)\mathrm{Both}\left(1\right)\mathrm{and}\left(3\right)$

_{2}react with 2 mol of O_{2}in a two-litre container to form one mole of NO. What will be the number of moles of O_{2}per litre at equilibrium?(1) 0.75 (2) 1.50 (3) 1.25 (4) None of the above

Ans: A.

How?

$\mathbf{40}\mathbf{.}\mathbf{}\text{'}a\text{'}molofPC{l}_{5},undergoes,thermaldissociationas:\phantom{\rule{0ex}{0ex}}PC{l}_{5}\rightleftharpoons PC{l}_{3}+C{l}_{2},themolefractionofPC{l}_{3}atequilibriumis0.25andthetotalpressureis2.0atm.TheparticalpressureofC{l}_{2}atequilibriumis:-\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\left(1\right)2.5\left(2\right)1.0\left(3\right)0.5\left(4\right)None$

6.5 Calculate Kp for the reaction, c(s) + H20 (g) CO(g) + H2(g) 6.13 at 990 K if the equilibrium concentrations are as 6.14 ca follows : [H20] = 1.10M, [COI = = 0.2M, R = 0.08206 L atm mor . 6.15 (Hint : First calculate Kc) (Kp 2.954) 6.6 The equilibrium constant Kc for the reaction —-—-.y 2NH3 (g) is 0.286 at 5000C. Calculate Kc and Kp for the 6.1t

(R = 0.08 l-atm/K-mol)

(a) 2430

(b) 1420

(c) 845

(d) 1002

Asap